Measuring Rate Reaction (Experimental Data) Determining and Using an Initial Rate of Reaction. Your Turn! In the reaction 2 NO(g) + Cl2(g) → 2NOCl(g) What is the rate of reaction with respect to NO? D A. What would be the rate of disapperance O 2? A.The same B.Twice as great C.Half as large D.You cannot tell from the given information 11 Your Turn! Based on the reaction 2CO(g) + O2(g) → 2CO2(g) the rate of disappearance CO is measured to be 2.0 M/s. Rate reaction Always positive Whether is 10 increasing or decreasing Rate of reaction = rate of disappearance of reactants 1 Δ 1 Δ =b Δt a Δt = rate of appearance of products =Ģ Fe3+(aq) + Sn2+ → 2 Fe2+(aq) + Sn4+(aq) 1 Δ Δ 1 Δ = Δt Δt 2 Δt 2 Measuring Rate Reaction Rate of change of concentration with time. Chemicals that participate in mechanism but are regenerated at the end.Substances that increase rates of chemical reactions without being used up.Most reactions, even exothermic reactions, require energy to occur Faster molecules collide more often and collisions have more energy b. Raising temperature usually makes reaction faster : a.Rates are often very sensitive to temperature.Collision rate between A and B increase if we increase or increase.Rates of both homogeneous and heterogeneous reactions affected by.Reactants in different phases Reactants meet only at interface between phases Surface area determines reaction rate Increase area, increase rate decrease area, decrease rate Ability of reactants to come in contact Reactants must meet in order to react What are fundamental differences in chemical reactivity?Ģ.What elements, compounds, salts are involved?.How quickly reactants disappear and products form 4.Write the reaction mechanism and decide which the most possible mechanism using experimental data.Calculates activation energy from Arrhenius equation.Determines rate laws of zero, 1st, and 2nd order.Calculates the relative rate of reactant reduction and the addition of product from the experimental data.Describes factors that affect reaction rates.Petrucci et.al, 9ed, 2007, Prentice-Hall © Raymond Chang, Chemistry, 10 ed, 2010, McGraw Hill. Chemical Kinetics References: Brady/Jespersen/Hyslop, Chemistry, 7 ed, 2015, John Wiley & Sons, Inc.
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